ENVIRONMENTAL CHEMISTRY Vol. 33 No. 5 May 2014 DOI /j. issn * 1,2 郭广亮 1,3** 王崇臣王 1 鹏

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1 ENVIRONMENTAL CHEMISTRY Vol 33 No 5 May 2014 DOI /j issn * 1,2 郭广亮 1,3** 王崇臣王 1 鹏 K Langmuir Freundlich Dubinin-Radushkevish Web-Morris Gibbs!G 0!H 0!S 0 Langmuir Gibbs!G 0 0!H 0!S 0 0 k g mg - 1 min - 1 Web-Morris Adsorption of acid fuchsin on biopottery Kinetic and thermodynamic studies GUO Guangliang 1 2 WANG Chongchen 1 3** WANG Peng 1 1 Key Laboratory of Urban Storm Water System and Water Environment Beijing University of Civil Engineering and Architecture Beijing China 2 Beijing Climate Change Response Research and Education Center Beijing University of Civil Engineering and Architecture Beijing China 3 The College of Materials Science and Engineering Beijing University of Technology Beijing China Abstract In order to investigate the dye adsorption properties of biopottery acid fuchsin was chosen as the sorbate The data obtained from different temperature K were fitted with Langmuir Freundlich and Dubinin-Radushkevish models to describe the equilibrium isotherms The kinetics rates were modeled using pseudo-first-order and pseudo-second-order kinetic equations Using web-morris model to explore mechanisms for adsorption kinetics The Gibbs free energy!g 0 enthalpy change!h 0 and entropy change!s 0 were calculated The results revealed that the equilibrium adsorption amount increased with the increase of temperature The adsorption could be well depicted by the Langmuir adsorption isotherm The Gibbs free energy!g 0 was negative while enthalpy change!h 0 and entropy change!s 0 were both positive indicating that the adsorption was a spontaneous endothermic and increasing entropy process The adsorption kinetics followed pseudo-second-order kinetic equation the rate k 2 was g mg - 1 min - 1 Web-Morris model can well explain the mechanism of adsorption kinetics and the intra-particle diffusion controls the adsorption rate * 2013M CIT&CD D B KZ ** Tel chongchenwang@ 126 com

2 Keywords biopottery acid fuchsin adsorption thermodynamics kinetics nm m 2 g ml g S SHZ-82 Spectrum SEM Zetasizer Nano C 20 H 17 N 3 Na 2 O 9 S Spectrum cm - 1 KBr SEM 0 02 g 20 ml 10 min 200 Zetasizer Nano Zeta ml 0 6 g L ml mg L K 150 r min μm 545 nm A q = C 0 - C e V W 1 η = C 0 - C e 100% 2 C 0 q mg g - 1 C 0 mg L - 1 C e mg L - 1 V L W g η g L mg L K 0 45 μm 3 0 ml

3 5 807 A Langergren Weber-Morris 5 6 ln( q e - q ) t = ln q e - k 1 t 3 t = t 4 q t k 2 q 2 q e e q t = k 3 t 1 /2 + b 5 q e q t t mg g - 1 k 1 min - 1 k 2 g mg - 1 min - 1 k 3 mg g - 1 min - 1 /2 b ml mg L g L K 150 r min - 1 q e K Langmuir Freundlich Dubinin-Radushkevish C e q e = 1 q max K L + C e q max 6 lnq e = lnk F + 1 n lnc e 7 ( ) e lnq e = lnq max - K DR ε 2 ε = RTln C q e mg g - 1 q max mg g - 1 K L Langmuir L mg - 1 K F L mg - 1 n L g - 1 C e mg L - 1 ε polenyi K DR L mg - 1 E E = ( 2K ) DR ΔG 0 ΔH 0 ΔS 0 8 ΔG 0 = - RTlnK L 9 lnk D = ΔS 0 /R - ΔH 0 /RT 10 R J mol - 1 K - 1 T K K L Langmuir L mg ΔG 0 10 K D = q e /C e lnq e /C e q e q e 0 lnk D lnk D 1 /T ΔH 0 ΔS cm - 1 OH NH 14 cm cm - 1 OH 1417 cm cm cm cm cm - 1 OH 1000 cm

808 33 Fig 1 1 Infrared spectra of biopottery before and after acid fuchsin adsorption Fig 2 2 SEM SEM photograph of biopottery 2 1 3 Zeta ph Zeta - 19 7 mv - 19 6 mv 2 2 T = 308 K 100 150 200 mg L -

4 Fig 1 1 Infrared spectra of biopottery before and after acid fuchsin adsorption Fig 2 2 SEM SEM photograph of biopottery Zeta ph Zeta mv mv 2 2 T = 308 K mg L g L - 1 t q η 3 q q q η η Fig g L - 1 The removal efficiency of acid fuchsin with different initial concentration as a function of adsorption time the biopottery amount is fixed to 0 6 g L Langergren Weber-Morris 5

5 R 2 = K 2 = g mg - 1 min - 1 q e mg g - 1 q e mg g Fig 4 4 a b Kinetics equation fitting curve a Pseudo-first order kinetics b Pseudo-second order kinetics 5 q t t 1 /2 t 1 / mg L - 1 k mg g - 1 min - 1 /2 Fig 5 5 Intra-particle diffusion plots for the adsorption of acid fuchsin on biopottery Langmuir Freundlich Dubinin-Radushkevish D-R 6 Langmuir 2 1 Langmuir 1 Langmuir R Langmuir K L q max

6 R L R L = 1 / 1 + K L C 0 11 K L Langmuir C 0 mg L - 1 R L 0 1 R L 1 R L = 1 R L = R L 0 1 Fig 6 6 Langmuir Langmuir isotherms for the adsorption of acid fuchsin on biopottery Table 1 1 Langmuir Freundlich D-R Fitting parameters of Langmuir Freundlich and D-R isotherms for acid fuchsin adsorption by biopottery powder at different temperatures T /K q max / K L / mg g - 1 L mg - 1 Langmuir Freundlich D-R R 2 K F / K 1 /n R 2 DR / q max / L mg - 1 L mg - 1 mg g R 2 Freundlich Freundlich Freundlich n 1 /n /n D-R ΔG 0 ΔH 0 ΔS 0 lnk D 1 /T R 2 = ΔH 0 ΔS 0 2 Table 2 2 Values of thermodynamic parameters for the adsorption of acid fuchsin by biopottery /K K L / L mg - 1 ΔG 0 / kj mol - 1 ΔS 0 / J mol - 1 K - 1 ΔH 0 / kj mol

7 ΔG 0 0 ΔH 0 ΔS 0 0 ΔG kj mol - 1 ΔG kj mol - 1 ΔG kj mol ΔH 0 > 0 ΔH 0 30 kj mol ΔS 0 > Web-Morris 3 ΔG 0 0 ΔH 0 ΔS Xue F Zhang Y New progress of the researches on dyeing wast water treatment techniques J Water Science and Engineering Technology Nethaji S Sivasamy A Thennarasu G et al Adsorption of malachite green dye onto activated carbon derived from borassus aethiopum flower biomass J Journal of Hazardous Materials TiO 2 J Dong L Zinin P V Cowen J P et al Iron coated pottery granules for arsenic removal from drinking water J Journal of Hazardous Materials J J J Gadd M Biosorption Critical review of scientific rationale environmental importance and significance for pollution treatment J Journal of Chemical Technology and Biotechnology J Rao M Ramesh A Rao G PC et al Removal of copper and cadmium from the aqueous solutions by activated carbon derived from Ceiba pentandra hulls J Journal of Hazardous Materials / Sawalha M F Jose R Jaime R G Thermodynamics and isotherm studies of biosorption of Cu Pband Zn by leave of saltbush J The Journal of Chemical Thermodynamics Aksu Z D nmezg Binary biosorption of cadmium II and nickel II onto dried Chlorella vulgaris Co-ion effect on mono-component isotherm parameters J Process Biochemistry Chen X Lv S Liu S et al Adsorption of methylene blue by rice hull ash J Separation Science and Technology Celekli A Tanr verdi B Predictive modeling of removal of Lana set Red G on Characontraria kinetic equilibrium and thermodynamic studies J Chemical Engineering Journal Senthil K P Ramalingam S Senthamarai C et al Adsorption of dye from aqueous solution by cashew nut shell Studies on equilibrium isotherm kinetics and thermodynamics of interactions J Desalination Hidalgo N Mangiameli G Manzano T et al Oxidation and removal of industrial textile dyes by a novel peroxidase extracted from postharvest lentistubble J Biotechnology and Bioprocess Engineering

ph ph ph Langmuir mg /g Al 2 O 3 ph 7. 0 ~ 9. 0 ph HCO - 3 CO 2-3 PO mg /L 5 p

ph ph ph Langmuir mg /g Al 2 O 3 ph 7. 0 ~ 9. 0 ph HCO - 3 CO 2-3 PO mg /L 5 p 1 2 1 2 3 1 2 1. 100054 2. 100054 3. 100036 ph ph ph Langmuir 166. 67 mg /g Al 2 O 3 ph 7. 0 ~ 9. 0 ph HCO - 4 5. 00 mg /L 5 ph doi 10. 13928 /j. cnki. wrahe. 2017. 03. 017 TV213. 4 + TU991. 26 + 6 A 1000-0860

ENVIRONMENTAL CHEMISTRY Vol. 33 No. 5 May 2014 DOI /j. issn * 1,2 郭广亮 1,3** 王崇臣 王 1 鹏

ENVIRONMENTAL CHEMISTRY Vol. 33 No. 5 May 2014 DOI /j. issn * 1,2 郭广亮 1,3** 王崇臣王 1 鹏